Achieve Homework Week 2,3,4 #19 [ENDORSED]

[Allison Mercado-3F]

I was just wondering what the A stands for and if I use Heisenberg's uncertainty principle.
What is the minimum uncertainty in an electron's velocity (Δvmin)
if the position is known within 13 Å.
Thank you!

[Jocelyn Chin 1K]

A stands for Angstrom. It's a unit of measurement that's used mostly for atoms because it's super small, and you can find the conversion on the equation sheet (1A = 10^-10m). And yes, you would use the Heisenberg's uncertainty principle! You just need to make sure to convert the angstrom into meters.

[Marleena]

Hi! The A is equivalent to 10^-10 meters. This is provided for us during the text under the constants and equations worksheet. And yes I used Heisenberg's principle!

[Barbara Soliman 1G]

The A stands for Angstrom. 1 A is equal to 10^-10 meters. Hope this helps!

[Reagan Feldman 1D]

To reiterate, the A stands for Angstroms, and this conversion can be found on the constants and equations sheets. (1A= 10^-10 m). You would still use Heisenberg's uncertainty principle for this problem and calculate the same way, just be sure keep the units consistent and convert from Angstroms to meters.

[Allison Mercado-3F]

Thank you for the help! How would I determine the uncertainty for a helium atom like in the second part of the problem?

[Ruben Adamov 1E]

So the uncertainty equation is: delta p * delta x >= h/4*pi. (delta p = m* delta v)
In the problem you are given the position(delta x) at 1 A. Convert this to meters first. You also know the atomic weight of He (4.0026 g/mol). To solve this problem you should convert g/mol to kg/atom. After you have all given values in correct units plug it in to the equation and solve for delta v.

[Sarah Hong 2K]

A stands for Angstrom and 1 A is equal to 10^-10 meters.